Question

With an activity show that lighter gases are diffuse faster than heavier gases .Describe an expression between their rates and molecular mases

Answer 1

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Answer 2

Explanation:

According to Graham's law, the rate of diffusion or effusion of two gases is inversely proportional to the square root of their respective molar masses.

Mathematically,  $\frac{R_{1}}{R_{2}} = \sqrt{\frac{M_{2}}{M_{1}}}$

where   $R_{1}$ = rate of effusion or diffusion of first gas

             $R_{2}$ = rate of effusion or diffusion of second gas

            $M_{1}$ = molar mass of first gas

             $M_{2}$ = molar mass of second gas

An activity to show that lighter gases are diffuse faster than heavier gases  is as follows.

Take a glass tube with a hole on each left and right side. From the left hole pass HCl gas and from the right hole pass ammonia ($NH_{3}$) gas. The ammonia gas is lighter than HCl gas, so it will expand rapidly inside the glass tube. Whereas HCl gas being heavier will not expand readily.

When both ammonia and HCl gas will mix then there will be formation of ammonium chloride which can be seen as white fumes.

Since HCl gas is heavier so, ammonium chloride will be formed closer to the release point of HCl gas.